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1 of 52 AP Chem 2013-2014 Summer Assignment (2549892) Question 12345678910111213141516171819202122232425262728293031323334353637 Description Problems from Chapters 1-3 of Zumdahl Instructions The following questions represent the baseline knowledge you will need to succeed in AP Chemistry. The goal of this assignment is twofold. First, it will tell you what you are up against in the upcoming school year. Second, this assignment covers curriculum that is basic and will allow us the time to cover more critical material in class during the school year. We will review this material during the first week of school and you will be tested on it at the end of the second week of school. Answer the following questions before the beginning of the 2013-2014 school year. If you have questions, please feel free to email me at [email protected]. If you would like to pick up a textbook from school to help you with this, send me an email but you have access to the digital text. I give you the answers for all questions so you know when you get it correct. You don't have to show work for the naming questions....just know the answers BUT you do have to hand in work for the math-based questions. 1. Question Details ZumChem8 1.E.097. [1070250] A column of liquid is found to expand linearly on heating 5.40 cm for a 12.7°F rise in temperature. If the initial temperature of the liquid is 95.3°F, what will the final temperature be in °C if the liquid has expanded by 20.0 cm? 61.3 °C - 2 of 52 2. Question Details ZumChem8 1.E.099. [1068700] For each of the following, decide which block is more dense: the orange block, the blue block, or it cannot be determined. (a) orange blue cannot be determined Explain your answer. Key: Volume density = mass; the orange block is more dense. Since mass (orange) > mass (blue) and since volume (orange) < volume (blue), the density of the orange block must be greater to account for the large mass of the orange block. - 3 of 52 (b) orange blue cannot be determined Explain your answer. Key: Which block is more dense cannot be determined. Since mass (orange) > mass (blue) and since volume (orange) > volume (blue), the density of the orange block may or may not be greater than the blue block. If the blue block is more dense, it's density cannot be so large that it's mass is larger than the orange block's mass. (c) 4 of 52 orange blue cannot be determined Explain your answer. Key: Since mass (blue) = mass (orange) and since volume (blue) < volume (orange), the density of the blue block must be larger in order to equate the masses. (d) orange blue cannot be determined Explain your answer. 5 of 52 Key: Since mass (blue) > mass (orange) and since the volumes are equal, the density of the blue block must be larger in order to give the blue block the larger mass. 3. Question Details ZumChem8 1.E.105. [1864423] - Many times errors are expressed in terms of percentage. The percentage error is the absolute value of the difference of the true value and the experimental value, divided by the true value, and multiplied by 100. Calculate the percent error for the following measurements. (a) The density of an aluminum block determined in an experiment was 2.61 g/cm3. (True value 2.70 g/cm3.) 3 % (b) The experimental determination of iron in iron ore was 16.60%. (True value 16.12%.) 3.0 % (c) A balance measured the mass of a 1.000 g standard as 0.9911 g. 0.9 % 4. Question Details ZumChem8 1.E.112. [1070254] An experiment was performed in which an empty 100 mL graduated cylinder was weighed. It was weighed once again after - 6 of 52 it had been filled to the 10.0 mL mark with dry sand. A 10 mL pipet was used to transfer 10.00 mL of methanol to the cylinder. The sand-methanol mixture was stirred until bubbles no longer emerged from the mixture and the sand looked uniformly wet. The cylinder was then weighed again. Use the data obtained from this experiment (and displayed at the end of this problem) to find the density of each of the following. Mass of cylinder plus wet sand 45.2613 g Mass of cylinder plus dry sand 37.3488 g Mass of empty cylinder 22.8317 g Volume of dry sand 10.0 mL Volume of sand + methanol 17.6 mL Volume of methanol 10.00 mL dry sand 1.45 g/mL methanol 0.7913 g/mL sand particles 1.9 g/mL Does the bubbling that occurs when the methanol is added to the dry sand indicate that the sand and methanol are reacting? Yes No 5. Question Details ZumChem8 1.E.072. [1070253] - 7 of 52 A copper wire (density = 8.96 g/cm3) has a diameter of 0.10 mm. If a sample of this copper wire has a mass of 25 g, how long is the wire? 1200 ft 6. Question Details ZumChem8 1.E.069. [1068689] In each of the following pairs, which has the greater volume? (a) lead or feathers 1.0 kg of lead 1.0 kg of feathers Both have same volume. (b) gold or water 100 g of gold 100 g of water Both have same volume. (c) mercury or copper 1.0 L of mercury 1.0 L of copper Both have same volume. - 8 of 52 7. Question Details ZumChem8 1.E.065. [1070257] - A sample containing 33.49 g of metal pellets is poured into a graduated cylinder initially containing 11.8 mL of water, causing the water level in the cylinder to rise to 19.1 mL. Calculate the density of the metal. 4.6 g/cm3 8. Question Details ZumChem8 1.E.056. [1092120] - Convert the following Kelvin temperatures to Celsius and Fahrenheit degrees. (a) the temperature that registers the same value on both the Fahrenheit and Celsius scales, 233 K -40. °C -40. °F (b) the boiling point of helium, 4K -269 °C -452 °F (c) the temperature at which many chemical quantities are determined, 298 K 25 °C 77 °F (d) the melting point of tungsten, 3680 K 3410 °C 6160 °F 9. Question Details ZumChem8 1.E.044. [1070243] - 9 of 52 Although the preferred SI unit of area is the square meter, land is often measured in the metric system in hectares (ha). One hectare is equal to 10,000 m2. In the English system, land is often measured in acres (1 acre = 160 rod2). Use the exact conversions and those given below to calculate the following. 5 1/2 yards = 1 rod 40 rods = 1 furlong 8 furlongs = 1 mile 0.01 km2 (a) 1 ha = (b) The area of a 4.5 acre plot of land in hectares, square meters, and square kilometers 1.8 ha 18000 m2 0.018 km2 (c) A lot with dimensions 120 ft by 75 ft is to be sold for $6500. What is the price per acre? $ 31000 What is the price per hectare? $ 10. Question Details 78000 ZumChem8 2.CW.03. [1110960] - 10 of 52 . 11 of 52 11. Question Details ZumChem8 2.E.061. [1212712] Would you expect each of the following atoms to gain or lose electrons when forming ions? What ion is the most likely in each case? (a) Na (b) Te gain gain lose ion formed lose ion formed Na+ Te2- (c) Rb (d) Br gain lose ion formed Rb+ gain lose ion formed Br- - 12 of 52 (e) O (f) Al gain gain lose lose ion formed ion formed O2- 12. Al3+ Question Details ZumChem8 2.E.060. [1212698] Complete the following table. Symbol 238 U Number of protons in nucleus 92 Number of neutrons in nucleus 146 Number of electrons 92 Net charge 0 - 13 of 52 92 40 Ca2+ 20 20 20 51 3+ V 23 23 28 89 39 Y 79 Br35 31 3P 15 39 18 20 50 35 44 15 16 2+ 3+ -or- +3 39 36 0 1- -or- -1 -or- - 18 3- 14 of 52 13. Question Details ZumChem8 2.E.064. [1212707] Name the compounds in parts (a) through (d) and write the formulas for the compounds in parts (e) through (h). (Enter your answer using the format copper(II) chloride for CuCl2.) (a) TiCl4 titanium(IV) chloride (b) FeBr3 iron(III) bromide (c) CoS cobalt(II) sulfide (d) Hg2O mercury(I) oxide (e) tin(II) nitride Sn3N2 - 15 of 52 (f) mercury(II) oxide HgO (g) niobium(V) oxide Nb2O5 (h) iron(III) oxide Fe2O3 14. Question Details ZumChem8 2.E.067. [1068708] Name each of the following compounds. (a) K2Cr2O7 potassium dichromate - 16 of 52 (b) NaClO2 sodium chlorite (c) Li3PO4 lithium phosphate (d) BaSO3 barium sulfite 15. Question Details ZumChem8 2.E.066. [1214701] Write the formula for each of the following compounds. (a) aluminum sulfide Al2S3 (b) beryllium oxide BeO (c) potassium bromide - 17 of 52 KBr (d) tin(IV) fluoride SnF4 (e) magnesium chloride MgCl2 (f) silver iodide AgI 18 of 52 16. Question Details ZumChem8 2.E.069. [1068688] - ZumChem8 2.E.072. [1068691] - Name each of the following compounds. (a) SO2 sulfur dioxide (b) N2O4 dinitrogen tetroxide (c) dinitrogen tetroxide (d) iodine trichloride 17. Question Details Name each of the following compounds. Assume the acids are dissolved in water. (Enter your answer using the format copper(II) chloride for CuCl2.) (a) HC2H3O2 acetic acid (b) NH4NO2 ammonium nitrite 19 of 52 (c) Co2S3 cobalt(III) sulfide (d) ICl iodine monochloride (e) Pb3(PO4)2 lead(II) phosphate (f) KClO3 potassium chlorate (g) H2SO4 sulfuric acid (h) Sr3N2 strontium nitride (i) Al2(SO3)3 aluminum sulfite (j) SnO2 tin(IV) oxide -or- stannic oxide (k) Na2CrO4 sodium chromate (l) HClO hypochlorous acid 20 of 52 18. Question Details ZumChem8 2.E.075. [1212693] Write the formula for each of the following compounds. (a) sulfur difluoride SF2 (c) sodium dihydrogen phosphate NaH2PO4 (e) chromium(III) carbonate Cr2(CO3)3 (b) sulfur hexafluoride SF6 (d) lithium nitride Li3N (f) tin(II) fluoride SnF2 - 21 of 52 (g) ammonium acetate NH4C2H3O2 (i) cobalt(III) nitrate Co(NO3)3 (k) potassium chlorate KClO3 19. Question Details (h) ammonium hydrogen sulfate NH4HSO4 (j) mercury(I) chloride Hg2Cl2 (l) sodium hydride NaH ZumChem8 2.E.105. [1068719] Each of the following statements is true, but Dalton might have had trouble explaining some of them with his atomic - 22 of 52 theory. Give explanations for the following statements. (a) The space-filling models for ethyl alcohol and dimethyl ether are shown below. These two compounds have the same composition by mass (52% carbon, 13% hydrogen, and 35% oxygen), yet the two have different melting points, boiling points, and solubilities in water. Key: Both compounds have C2H6O as the formula. Because they have the same formula, their mass percent composition will be identical. However, these are different compounds with different properties since the atoms are bonded together differently. These compounds are called isomers of each other. (b) Burning wood leaves an ash that is only a small fraction of the mass of the original wood. Key: When wood burns, most of the solid material in wood is converted to gases, which escape. The gases produced are most likely CO2 and H2O. (c) Atoms can be broken down into smaller particles. 23 of 52 Key: The atom is not an indivisible particle, but is instead composed of other smaller particles, e.g., electrons, neutrons, and protons. (d) One sample of lithium hydride is 87.4% lithium by mass, while another sample of lithium hydride is 74.9% lithium by mass. However, the two samples have the same properties. Key: The two hydride samples contain different isotopes of either hydrogen and/or lithium. Although the compounds are composed of different isotopes, their properties are similar because different isotopes of the same element have similar properties (except, of course, their mass). 20. Question Details ZumChem8 2.E.095. [1212690] The designations 1A through 8A used for certain families of the periodic table are helpful for predicting the charges on ions in binary ionic compounds. In these compounds, the metals generally take on a positive charge equal to the family number, while the nonmetals take on a negative charge equal to the family number minus eight. Thus the compound between sodium and chlorine contains Na+ ions and Cl- ions and has the formula NaCl. Predict the formula and the name of the binary compound formed from the following pairs of elements. elements formula name - 24 of 52 (a) Ca and N Ca3N2 calcium nitride (b) K and O K2 O potassium oxide (c) Rb and F RbF rubidium fluoride (d) Mg and S MgS magnesium sulfide (e) Ba and I BaI2 barium iodide 25 of 52 21. (f) Al and Se Al2Se3 aluminum selenide (g) Cs and P Cs3P cesium phosphide (h) In and Br InBr3 indium(III) bromide Question Details ZumChem8 2.E.090. [1212695] For each of the following ions, indicate the total number of protons and electrons in the ion. For the positive ions in the list, predict the formula of the simplest compound formed between each positive ion and the oxide ion. For the negative ions in the list, predict the formula of the simplest compound formed between each negative ion and the aluminum ion. (b) Se2- (a) F ‾ protons 9 protons 34 - 26 of 52 electrons compound 10 AlF3 electrons compound 36 Al2Se3 (d) Rb+ (c) Fe2+ protons 26 protons 37 electrons 24 electrons 36 compound compound FeO (e) Mg2+ Rb2O (f) Fe3+ protons 12 protons 26 electrons 10 electrons 23 27 of 52 compound compound MgO (g) Cr3+ (h) Br‾ protons 24 protons 35 electrons 21 electrons 36 compound 22. Fe2O3 Cr2O3 compound Question Details AlBr3 ZumChem8 3.E.170. [1865488] The compound As2I4 is synthesized by reaction of arsenic metal with arsenic triiodide. If a solid cubic block of arsenic (d = 5.72 g/cm3) that is 3.18 cm on edge is allowed to react with 1.01 1024 molecules of arsenic triiodide, how much As2I4 can be prepared? 827 g If the percent yield of As2I4 was 73.7%, what mass of As2I4 was actually isolated? - 28 of 52 609 g 23. Question Details ZumChem8 3.E.151. [1214718] - A compound contains only carbon, hydrogen, nitrogen, and oxygen. Combustion of 0.157 g of the compound produced 0.213 g CO2 and 0.0310 g H2O. In another experiment, it is found that 0.103 g of the compound produces 0.0230 g NH3. What is the empirical formula of the compound? Hint: Combustion involves reacting with excess O2. Assume that all the carbon ends up in CO2 and all the hydrogen ends up in H2O. Also assume that all the nitrogen ends up in the NH3 in the second experiment. C 7H5N 3O 6 24. Question Details ZumChem8 3.E.152. [1053089] - Nitric acid is produced commercially by the Ostwald process, represented by the following equations. 4 NH3(g) + 5 O2(g) 2 NO(g) + O2(g) 3 NO2(g) + H2O(l) 4 NO(g) + 6 H2O(g) 2 NO2(g) 2 HNO3(aq) + NO(g) What mass in kg of NH3 must be used to produce 4.5 106 kg HNO3 by the Ostwald process, assuming 100% yield in each reaction? 1.8e+06 kg 25. Question Details ZumChem8 3.E.154. [1092133] A 9.752-g gaseous mixture contains ethane (C2H6) and propane (C3H8). Complete combustion to form carbon dioxide and - 29 of 52 water requires 1.120 mol of oxygen. Calculate the mass percent of ethane in the original mixture. (Use 1.008, 12.01, and 16.00 amu as the atomic mass for hydrogen, carbon, and oxygen, respectively.) 48.3 % 26. Question Details ZumChem8 3.E.135. [1053046] - The empirical formula of styrene is CH; the molar mass of styrene is 104.14 g/mol. What number of H atoms are present in a 9.00 g sample of styrene? 4.16e+23 atoms 27. Question Details ZumChem8 3.E.136. [1214692] - Terephthalic acid is an important chemical used in the manufacture of polyesters and plasticizers. It contains only C, H, and O. Combustion of 23.77 mg terephthalic acid produces 50.38 mg CO2 and 7.74 mg H2O. If 0.250 mol of terephthalic acid has a mass of 41.5 g, determine the molecular formula of terephthalic acid. C 8H6O 4 28. Question Details ZumChem8 3.E.138. [1053092] A binary compound between an unknown element E and hydrogen contains 91.27% E and 8.73% H by mass. If the formula of the compound is E3H8, calculate the atomic mass of E. 28.1 amu - 30 of 52 29. Question Details ZumChem8 3.E.140. [1053070] - ABS plastic is a tough, hard plastic used in applications requiring shock resistance. The polymer consists of three monomer units: acrylonitrile (C3H3N), butadiene (C4H6), and styrene (C8H8). (a) A sample of ABS plastic contains 8.80% N by mass. It took 0.605 g of Br2 to react completely with a 1.20 g sample of ABS plastic. Bromine reacts 1:1 (by moles) with the butadiene molecules in the polymer and nothing else. What is the percent by mass of acrylonitrile and butadiene in this polymer? C3H3N 33.3 % C4H6 17.1 % (b) What are the relative numbers of each of the monomer units in this polymer? (Give the ratio of acrylonitrile:butadiene:styrene. Use the lowest possible coefficients.) 4 (C3H3N) : 30. 2 (C4H6) : 3 (C8H8) Question Details ZumChem8 3.E.142. [1216940] Methane (CH4) is the main component of marsh gas. Heating methane in the presence of sulfur produces carbon disulfide and hydrogen sulfide as the only products. (a) Write the balanced chemical equation for the reaction of methane and sulfur. (Use the lowest possible coefficients. Include states of matter under SATP conditions in your answer.) CH4(g) + 4 S(s) → CS2(l) + 2 H2S(g) -or- 2 CH4(g) + S8(s) → 2 CS2(l) + 4 H2S(g) (b) Calculate the theoretical yield of carbon disulfide when 160. g of methane is reacted with an equal mass of - 31 of 52 sulfur. 95.0 g 31. Question Details ZumChem8 3.E.146. [1053064] - Commercial brass, an alloy of Zn and Cu, reacts with hydrochloric acid as follows. Zn(s) + 2 HCl(aq) ZnCl2(aq) + H2(g) (Cu does not react with HCl.) When 0.5133 g of a certain brass alloy is reacted with excess HCl, 0.0985 g ZnCl2 is eventually isolated. (a) What is the composition of the brass by mass? Zn 9.21 % Cu 90.79 % (b) How could this result be checked without changing the above procedure? Key: The Cu remains unreacted. After filtering, washing, and drying, the mass of the unreacted copper could be measured. 32. Question Details ZumChem8 3.E.116. [1053063] Consider the following unbalanced reaction. P4(s) + F2(g) PF3(g) What mass of F2 is needed to produce 220. g of PF3 if the reaction has a 74.2% yield? - 32 of 52 192 g 33. Question Details ZumChem8 3.E.115. [1053080] - Bornite (Cu3FeS3) is a copper ore used in the production of copper. When heated, the following reaction occurs. 2 Cu3FeS3(s) + 7 O2(g) 6 Cu(s) + 2 FeO(s) + 6 SO2(g) If 3.48 metric tons of bornite is reacted with excess O2 and the process has an 78.0% yield of copper, what mass of copper is produced? 1.51 metric tons 34. Question Details ZumChem8 3.E.104. [1053067] - Phosphorus can be prepared from calcium phosphate by the following reaction. 2 Ca3(PO4)2(s) + 6 SiO2(s) + 10 C(s) → 6 CaSiO3(s) + P4(s) + 10 CO(g) Phosphorite is a mineral that contains Ca3(PO4)2 plus other non-phosphorus-containing compounds. What is the maximum amount of P4 that can be produced from 2.1 kg of phosphorite if the phosphorite sample is 99% Ca3(PO4)2 by mass? Assume an excess of the other reactants. 420 g 35. Question Details ZumChem8 3.E.102. [1216955] One of relatively few reactions that takes place directly between two solids at room temperature is given in the equation below. In this equation, the · 8 H2O in Ba(OH)2 · 8 H2O indicates the presence of eight water molecules. This compound is called barium hydroxide octahydrate. (a) Balance the equation. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) - 33 of 52 Ba(OH)2 · 8 H2O(s) + NH4SCN(s) → Ba(SCN)2(s) + H2O(l) + NH3(g) Ba(OH)2 . 8 H2O(s) + 2 NH4SCN(s) → Ba(SCN)2(s) + 10 H2O(l) + 2 NH3(g) (b) What mass of ammonium thiocyanate (NH4SCN) must be used if it is to react completely with 4.8 g barium hydroxide octahydrate? 2.3 g 36. Question Details ZumChem8 3.E.089. [1214726] Give the balanced equation for each of the following chemical reactions. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) (a) Glucose (C6H12O6) reacts with oxygen gas to produce gaseous carbon dioxide and water vapor. C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(g) (b) Solid iron(III) sulfide reacts with gaseous hydrogen chloride to form solid iron(III) chloride and hydrogen sulfide gas. Fe2S3(s) + 6 HCl(g) → 2 FeCl3(s) + 3 H2S(g) - 34 of 52 (c) Carbon disulfide liquid reacts with ammonia gas to produce hydrogen sulfide gas and solid ammonium thiocyanate (NH4SCN). CS2(l) + 2 NH3(g) → H2S(g) + NH4SCN(s) 37. Question Details ZumChem8 3.E.095. [1216947] Balance the following equations representing combustion reactions. (Use the lowest possible coefficients. Include statesof-matter under the given conditions in your answer where appropriate.) (a) 2 (b) 2 (c) C12H22O11(s) + O2(g) + 15 + → 13 → CO2(g) + H2O(g) C12H22O11(s) + 12 O2(g) → 12 CO2(g) + 11 H2O(g) 12 → + 8 6 + 10 - 35 of 52 (d) Fe(s) + O2(g) → Fe2O3(s) 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) (e) FeO(s) + O2(g) → Fe2O3(s) 4 FeO(s) + O2(g) → 2 Fe2O3(s) 38. Question Details ZumChem8 3.E.088. [1214710] A compound contains only carbon, hydrogen, and oxygen. Combustion of 9.612 mg of the compound yields 14.41 mg CO2 and 3.93 mg H2O. The molar mass of the compound is 176.1 g/mol. What are the empirical and molecular formulas of the compound? empirical formula molecular formula C 3H4O 3 C 6H8O 6 - 36 of 52 39. Question Details ZumChem8 3.E.069. [1053082] - There are several important compounds that contain only nitrogen and oxygen. Calculate the mass percent of nitrogen in each of the following. (a) NO, a gas formed by the reaction of N2 with O2 in internal combustion engines. 46.7 % (b) NO2, a brown gas mainly responsible for the brownish color of photochemical smog. 30.4 % (c) N2O4, a colorless liquid used as a fuel in space shuttles. 30.4 % (d) N2O, a colorless gas sometimes used as an anesthetic by dentists (known as laughing gas). 63.7 % 40. Question Details ZumChem8 3.E.070. [1053090] - 37 of 52 Arrange the following substances in order of increasing mass percent of carbon. caffeine, C8H10N4O2 sucrose, C12H22O11 ethanol, C2H5OH ---Select--- 41. sucrose < ---Select--- caffeine < ---Select--- Question Details ethanol ZumChem8 3.E.071. [1061771] - Fungal laccase, a blue protein found in wood-rotting fungi, is 0.390% Cu by mass. If a fungal laccase molecule contains 4 copper atoms, what is the molar mass of fungal laccase? 65200 g/mol 42. Question Details ZumChem8 3.E.065. [1053083] Chloral hydrate (C2H3Cl3O2) is a drug formerly used as a sedative and hypnotic. It is the compound used to make "Mickey Finns" in detective stories. (a) Calculate the molar mass of chloral hydrate. 165 g/mol (b) What amount (moles) of C2H3Cl3O2 molecules are in 501.0 g chloral hydrate? 3.029 mol (c) What is the mass in grams of 2.0 10-2 mol chloral hydrate? 3.3 g (d) What number of chlorine atoms are in 4.4 g chloral hydrate? 4.8e+22 - 38 of 52 (e) What mass of chloral hydrate would contain 2.4 g Cl? 3.7 g (f) What is the mass of exactly 483 molecules of chloral hydrate? 1.33e-19 g 43. Question Details ZumChem8 3.E.064. [1053088] - Complete the following table. Sample Mass of sample (g) C6H6 4.28 H2O CO2 CH3OH 44. 4.32 1.85 0.297 Moles of sample (mol) Molecules in sample Total atoms in sample 0.0548 3.30e+22 3.96e+23 1.45e+23 4.34e+23 0.240 0.0420 0.00927 2.53 5.58e+21 Question Details For each chemical term, select the appropriate examples. (Select all that apply.) (a) homogeneous mixture 1022 7.59e+22 3.35 1022 ZumChem8 1.E.028. [1068721] - 39 of 52 oil and water mixture brass (Cu + Zn) coffee saltwater glucose pure carbon (b) heterogeneous mixture hydrogen gas book desk liquid mercury argon gas tree (c) compound 40 of 52 copper (Cu) glucose (C6H12O6) carbon dioxide (CO2) water (H2O) sodium chloride (NaCl) oxygen (O2) (d) element zinc fluorine chloroform ethanol copper diethyl ether (e) physical change 41 of 52 boiling water combustion of gasoline dry ice subliming freezing water melting a popsicle photosynthesis (f) chemical change boiling water combustion of gasoline dry ice subliming freezing water melting a popsicle photosynthesis 45. Question Details ZumChem8 1.E.030. [1068695] Indicate the number of significant figures in each of the following statements. (If the number is an exact number, as in 100 cm in a meter, then type "infinite" for the number of significant figures.) (a) One inch is approximately 2.5 cm. - 42 of 52 2 -or- two (b) This book is almost 1200 pages. 2 -or- two (c) One gallon is about 3.8 L. 2 -or- two (d) This boat is approximately 900.00 tons. 5 -or- five (e) A gram is exactly 1000 mg. infinite -or- infinite (f)A liter is approximately 1.059 qt. 4 -or- four 46. Question Details ZumChem8 1.E.033. [1070594] Round off each of the following numbers to the indicated number of significant digits and write the answer in standard scientific notation. (a) 0.00034177 to four digits 3.418e-04 (b) 107.645 102 to two digits 1.1e+04 (c) 17.0425 to three digits - 43 of 52 1.70e+01 (d) 3.322 105 to two digits 3.3e+05 47. Question Details ZumChem8 1.E.062. [1070251] A rectangular block has dimensions 2.9 cm 2.0 cm - 10.0 cm. The mass of the block is 645.0 g. (a) What is the volume of the block? 58 cm3 (b) What is the density of the block? 11 g/cm3 48. Question Details ZumChem8 2.E.054. [1212694] Write the atomic symbol (AZX) for each of the isotopes described below. (a) number of protons = 20, number of neutrons = 20 40 Ca 20 (b) the isotope of boron with mass number 10 - 44 of 52 10 B 5 (c) Z = 53, A = 132 132 I 53 (d) atomic number 29, number of neutrons = 36 65 Cu 29 (e) Z = 11, number of neutrons = 12 23 Na 11 45 of 52 (f) number of protons = 12, mass number 23 23 Mg 12 49. Question Details ZumChem8 2.E.056. [1068730] How many protons, neutrons, and electrons are in each of the following atoms or ions? Protons 62 28 Ni 34 28 Au 79 118 79 Co2+ 27 33 25 O2- 8 10 10 Tc3+ 43 54 40 1 2 0 79 27 18 8 97 43 3 1 Electrons 28 197 60 Neutrons H+ - 46 of 52 50. Question Details ZumChem8 2.E.091. [1068703] - The formulas and common names for several substances are given below. Give the systematic names for these substances. (Enter your answer using the format copper(II) chloride for CuCl2.) (a) sugar of lead, Pb(C2H3O2)2 lead(II) acetate (b) blue vitrol, CuSO4 copper(II) sulfate (c) quicklime, CaO calcium oxide (d) Epsom salts, MgSO4 magnesium sulfate (e) milk of magnesia, Mg(OH)2 magnesium hydroxide (f) gypsum, CaSO4 calcium sulfate (g) laughing gas, N2O dinitrogen monoxide -or- nitrous oxide 51. Question Details ZumChem8 3.E.007. [1053052] A new grill has a mass of 30.0 kg. You put 1.0 kg of charcoal in the grill. You burn all the charcoal and the grill has a mass - 47 of 52 of 30.0 kg. What is the mass of the gases given off? (Assume that the charcoal is pure carbon solid and that it burns completely in oxygen.) 3.7 kg 52. Question Details ZumChem8 3.E.009. [1053073] - You may have noticed that water sometimes drips from the exhaust of a car as it is running. Is this evidence that there is at least a small amount of water originally present in the gasoline? Yes No Explain. Key: Water, along with carbon dioxide, are products of the combustion of hydrocarbons (such as octane in gasoline). 53. Question Details ZumChem8 3.E.016. [1070595] Consider the equation below. 2A+B → A2B If you mix 2.2 mol of A with 2.2 mol of B, what amount (moles) of A2B can be produced? 1.1 moles - 48 of 52 54. Question Details ZumChem8 3.E.033. [1053069] - An element consists of 1.40% of an isotope with mass 203.973 amu, 24.10% of an isotope with mass 205.9745 amu, 22.10% of an isotope with mass 206.9759 amu, and 52.40% of an isotope with mass 207.9766 amu. Calculate the average atomic mass. 207.2 amu Identify the element (Give the symbol). Pb 55. Question Details ZumChem8 3.E.061. [1053057] - ZumChem8 3.E.063. [1070587] - What amount (moles) are represented by each of these samples? (a) 170.0 g Fe2O3 1.064 mol (b) 20.0 mg NO2 0.000435 mol (c) 1.8 1016 molecules of BF3 3.0e-08 mol 56. Question Details What number of atoms of nitrogen are present in 8.50 g of each of the following? (a) magnesium nitride 1.01e+23 atoms 49 of 52 (b) lead(II) nitrate 3.09e+22 atoms (c) glycine, C2H5O2N 6.82e+22 atoms (d) calcium nitrate 6.24e+22 atoms 50 of 52 57. Question Details ZumChem8 3.E.004. [1053085] - Nitrogen (N2) and hydrogen (H2) react to form ammonia (NH3). Consider a mixture of six nitrogen molecules and six hydrogen molecules in a closed container. Assuming the reaction goes to completion, what will the final product mixture be? number of NH3 molecules 4 number of N2 molecules 4 number of H2 molecules 0 Which of the following equations best represents this reaction? N2 + 3 H2 6 N2 + 6 H2 N2 + H2 4 NH3 + 4 N2 NH3 N + 3 H2 2 N2 + 6 H2 58. 2 NH3 NH3 4 NH3 Question Details ZumChem8 3.E.034. [1070582] An element "X" has five major isotopes, which are listed below along with their abundances. Percent Natural Abundance Mass (amu) 46 8.00% 45.952690 47 7.30% 46.951764 48 73.80% 47.947947 Isotope X X X - 51 of 52 49 5.50% 48.947841 50 5.40% 49.944792 X X Calculate the average atomic mass. 47.9 amu What is the element? Titanium -or- titanium -or- Ti 59. Question Details ZumChem8 3.E.099. [1053072] Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid-fuel rocket motors. The reaction is given below. Fe2O3(s) + 2 Al(s) 2 Fe(l) + Al2O3(s) What masses of iron(III) oxide and aluminum must be used to produce 20.0 g iron? iron (III) oxide 28.6 g aluminum 9.66 g What is the maximum mass of aluminum oxide that could be produced? 18.3 g Assignment Details Name (AID): AP Chem 2013-2014 Summer Assignment (2549892) Feedback Settings Submissions Allowed: 50 Before due date Category: Homework Question Score Code: Assignment Score Locked: No Publish Essay Scores - 52 of 52 Author: Mantas, Nicholas ( [email protected] ) Question Part Score Last Saved: Jun 3, 2013 10:45 AM EDT Mark Permission: Protected Help/Hints Randomization: Person Response Which graded: Last Save Work After due date Question Score Assignment Score Publish Essay Scores Key Question Part Score Solution Mark Add Practice Button Help/Hints Response